Synthesis of diacyl peroxide in aprotic solvent

ABSTRACT

This invention relates to a process for the synthesis of diacyl peroxide by contacting acyl halide and peroxide complex in compatible aprotic solvent substantially free of compounds oxidizable by the peroxide complex or the reaction products of organic acyl halide with peroxide complex.

FIELD OF THE INVENTION

[0001] This invention is in the field of the synthesis of diacylperoxide from acyl halide in compatible aprotic solvent.

BACKGROUND OF THE INVENTION

[0002] Diacyl peroxides are among the commonly used initiators in thecommercial production of polyolefins, particularly fluoroolefins, suchas tetrafluoroethylene. They may be represented as R—(C═O)—O—O—(C═O)—R.The peroxide decomposes to give R•, known as a free radical, whichreacts with olefin monomer to begin the polymerization cycle. Takingtetrafluoroethylene as an example:

R—(C═O)—O—O—(C═O)—R→2R—(C═O)—O•→2R•+2CO₂R•+CF₂=CF₂→R—CF₂—CF₂•R—CF₂—CF₂•+CF₂═CF₂→R—CF₂—CF₂—CF₂—CF₂•

[0003] The R group arising from the initiator is called an “endgroup” ofthe polymer.

[0004] The classical synthesis of diacyl peroxides is an aqueoussynthesis. An alkaline aqueous solution of hydrogen peroxide iscontacted with a water-immiscible solution of acid halide. Examples arefound in S. R. Sandler and W. Karo, (1974) Polymer Synthesis, Vol. 1,Academic Press, Inc., Orlando, Fla., p. 451 and U.S. Pat. No. 5,021,516.This is a reaction of two liquid phases, an aqueous phase and anonaqueous phase. Equation (1) shows the reaction:

2R—(C═O)X+H₂O₂+2NaOH→R—(C═O)—O—O—(C═O)—R+2NaX+2H₂O   (1)

[0005] From the stoichiometry of (1) it is clear that one mole ofhydrogen peroxide reacts with two moles of acyl halide to yield one moleof diacyl peroxide. The diacyl peroxide as it forms is taken up in thewater immiscible phase. By this means, exposure of the acyl halide andthe diacyl peroxide to the alkaline aqueous phase is minimized, which isdesirable because water hydrolyzes both the organic acyl halide startingmaterial and the diacyl peroxide product. Hydrolysis decreases yield andintroduces byproducts such as acids and peracids, which are impurities.At the end of the reaction, the water-immiscible solvent with the diacylperoxide dissolved in it is separated and dried, and purified asnecessary.

[0006] The use of sodium percarbonate and sodium perborate for aqueousand nonaqueous functional group oxidation in organic synthesis has beenreported (A. McKillop and W. R. Sanderson, Tetrahedron, vol. 51, no. 22,pp. 6145-6166, 1995; J. Muzart, Synthesis pp. 1325-1346, November 1995).Organic oxidation reactions using urea/hydrogen peroxide adduct inprotic and aprotic solvents is reported by M.S. Cooper, et al. Synlett,pp. 533-535, September 1990. Organic acids, acid anhydrides, and acylhalides are reagents and solvents in these reactions and peracids areproposed as intermediates in the oxidations. Formation of diacylperoxide as an undesirable byproduct of the reaction is discussed.

[0007] Japanese Patent 61152653 discloses the preparation of diacylperoxides by the mixing of acyl halides with sodium peroxide (Na₂O₂) inhalogenated solvent, followed by addition of water. Sodium peroxide mustbe handled carefully: it can react violently or explosively with organicmaterials, is hygroscopic, and absorbs carbon dioxide from air to formcompounds that can ignite if subjected to pressure or friction.Furthermore, sodium peroxide, being strongly basic, cannot be used withcompounds that are sensitive to bases.

[0008] A safe, economical, synthesis of diacyl peroxides in aproticsolvent using stable, easy to handle oxidizing agents, and proceeding inhigh yield is needed. Looking to the future, the need is greatest for aprocess that can be run in a nonflammable solvents such asfluorocarbons, chlorofluorocarbons, or certain hydrohalocarbons.

SUMMARY OF THE INVENTION

[0009] One form of this invention relates to a process for the synthesisof diacyl peroxide by contacting organic acyl halide and peroxidecomplex, in compatible aprotic solvent substantially free of compoundsoxidizable by the peroxide complex or by products of the reaction oforganic acid halide with peroxide complex. A second form of thisinvention relates to a process for the continuous synthesis of diacylperoxide by continuously contacting a feed stream comprised of organicacyl halide in a compatible aprotic solvent with a bed comprised ofperoxide complex, to form a product stream comprised of diacyl peroxidein compatible aprotic solvent, the compatible aprotic solvent beingsubstantially free of compounds oxidizable by peroxide complex or byproducts of the reaction of organic acid halide with peroxide complex.

DETAILED DESCRIPTION OF THE INVENTION

[0010] The present invention relates to a process for the synthesis oforganic peroxides by contacting organic acyl halides with peroxidecomplexes in compatible aprotic solvents. Surprisingly, it has beenfound that diacyl peroxides can be prepared in good yield, andfurthermore that yield improves when the peroxide complex is in molarexcess relative to the acyl halide, which is contrary to expectationsand to the teaching of the prior art, both of which would lead one topredict that diacyl peroxide yield would be depressed and peracid yieldenhanced, by excess peroxide.

[0011] Organic acyl halides are compounds that can be represented by thestructure R—(C═O)X. X represents halogen: fluorine, chlorine, bromine,or iodine. The most readily available acyl halides are generally acylchloride or acyl fluoride. R represents any organic group that iscompatible with one or more of the peroxide complexes useful forcarrying out this invention under reaction conditions. A compatible Rgroup is one that does not contain atoms or groups of atoms that aresusceptible to oxidation by or otherwise react with the otheringredients in the course of the reaction or in the reaction mixture togive undesirable products. R groups acceptable in the present inventioninclude aliphatic and alicyclic groups, these same groups with etherfunctionality, aryl groups and substituted aryl groups in which thesubstituents are compatible with one or more of the peroxide complexesof this invention under the conditions of the synthesis. The R group maybe partially or completely halogenated. If perhalogenated, the R groupmay have only one type of halogen, as with perfluorinated groups, or mayhave several types, as with, for example, chlorofluorinated groups.

[0012] The R group may also contain certain functional groups or atomssuch as —COOCH₃, —SO₂F, —CN, I, Br, or H. As stated above, the R groupis incorporated in the polymer at the end of the polymer chain, that is,as an endgroup. It is sometimes useful to be able to further react thepolymer through the endgroup with other molecules, for example, othermonomers or polymer, or to introduce ionic functionality in the endgroupto promote interaction with polar surfaces such as metals, metal oxides,pigments, or with polar molecules, such as water or alcohols, to promotedispersion. Some of the functional groups above, for example —COOCH₃ and—SO₂F (the fluorosulfonyl group) are susceptible to hydrolysis,especially base-catalyzed hydrolysis, and reaction with nucleophiles.However, because of the absence of an aqueous phase in a preferred formof this invention and of the specificity of the peroxide complexesuseful in carrying out this invention, these functional groups are notaffected and the diacyl peroxides corresponding to these acyl halidescan be made. The invention thereby provides novel acyl peroxidecompounds having at least one fluorosulfonyl group in at least one ofthe acyl constituents. Preferably, at least one of the acyl constituentsis derived from FSO₂CF₂(C═O)F. For example, from FSO₂CF₂(C═O)F, thenovel compound FSO₂CF₂(C═O)—O—O—(C═O)CF₂SO₂F,bis[perfluoro(fluorosulfonyl)acetyl] peroxide, can be made withouthydrolysis of the sulfonyl fluoride functionality to sulfonic acid. Itis thus a farther advantage of the processes according to thisinvention, that such hydrolysis-sensitive groups can be incorporated indiacyl peroxides and thereby introduced as endgroups in polymers.

[0013] In the synthesis of diacyl peroxide in accordance with thisinvention, no more than one organic acyl halide will normally be used.Although with more than one organic acyl halide the reaction wouldproceed satisfactorily, more than one diacyl peroxide would be made. Forexample, if two organic acyl halides are used, A—(C═O)X and B—(C═O)X,three diacyl peroxides would be expected: A—(C═O)—O—O—(C═O)—A,B—(C═O)—O—O—(C═O)—B, and A—(C═O)—O—O—(C═O)—B, a mixed diacyl peroxide.The ratio of the peroxides can be controlled to some extent by the orderof addition of the organic diacyl halides. Such a mixture of peroxidesis usually undesirable because different peroxides will generally havedifferent decomposition rates. However, if a mixed diacyl peroxide iswanted, the method of this invention may be used, followed if necessaryby separation or purification steps to reduce or remove accompanyingunwanted peroxides.

[0014] Diacyl peroxides in which the acyl group is a hydrocarbon groupcan be made according to this invention. These hydrocarbon diacylperoxides are useful for initiation of olefin polymerization, includingfluoroolefin polymerization when the presence of a hydrocarbon endgroupis acceptable or desirable. Isobutyryl peroxide is preferred when a lowtemperature hydrocarbon initiator is needed. It can be made fromisobutyryl halide, preferably isobutyryl chloride.

[0015] Synthesis of diacyl peroxides according to this invention isparticularly useful for making initiators for the polymerization offluoroolefins such as tetrafluoroethylene, hexafluoroproplyene,perfluoro(alkyl vinyl ethers), chlorotrifluoroethylene, vinylidenefluoride, and vinyl fluoride, either as homopolymers, or as copolymerswith each other or with other olefins, such as ethylene andperfluoroalkylethylenes. Fluoroolefin polymerization is susceptible tochain transfer if compounds with labile carbon-hydrogen bonds arepresent, so it is desirable that initiators be free of such bonds.Furthermore, because of the high temperatures at which fluoropolymersare processed and the conditions under which they are often used, thethermal and hydrolytic stability of the polymer endgroups is important.The R group of the initiator is one source of such endgroups. Therefore,except in cases where specific reactivity of polymer endgroups iswanted, in the interest of minimizing chain transfer activity of theinitiator and of providing endgroups with thermal and hydrolyticstability comparable to that of the polymer chain, it is desirable thatthe R group be free of bonds that are capable of chain transfer or thatare less thermally or hydrolytically stable than the polymer itself. Inpolymerizing fluoromonomers, perhalogenated R groups, and preferablyperfluorinated R groups, meet this requirement. Because etherfunctionality in halogenated and fluorinated organic groups has goodthermal and oxidative stability if the oxygen is between carbon atomsthat are perhalogenated or perfluorinated, or between carbon atoms thatare substituted with perhaloalkyl or perfluoroalkyl groups, such etherfunctionality is acceptable also.

[0016] It is a further advantage of diacyl peroxide synthesis inaccordance with this invention that fluoroorganic acyl halides, that is,acyl halides in which the R group is at least partially fluorinated, andparticularly perfluoroorganic acyl halides, are readily reacted to formthe corresponding diacyl peroxides. An example of a perfluoroorganicacyl halide for this invention is perfluoro(2-methyl-3-oxa-hexanoylfluoride), also known as hexafluoropropylene oxide (HFPO) dimer acidfluoride and as DAF. It has the formula:

CF₃CF₂CF₂OCF(CF₃)(C═O)F

[0017] Other suitable perfluoroorganic acyl halides includeCF₃CF₂CF₂(C═O)Cl (heptafluorobutyryl chloride) and CF₃CF₂(C═O)F(pentafluoropropionyl fluoride).

[0018] The peroxide complexes useful for carrying out this inventioninclude a) complexes of hydrogen peroxide with inorganic compounds,referred to here as inorganic complexes, and b) complexes of hydrogenperoxide with organic molecules, referred to here as organic peroxidecomplexes. These complexes include those substances in which hydrogenperoxide is combined with inorganic or organic compounds by bonds strongenough to permit isolation of the compounds, though the bonds may beweaker or of a different character than those between the constituentsof hydrogen peroxide or of the compound with which it is complexed. Bythis criterion it can be seen that “sodium percarbonate”, which isisolable and has the composition Na₂CO₃•1½H₂O₂, is a complex of hydrogenperoxide, while an aqueous solution of hydrogen peroxide, although itmay have degrees of hydration that vary with concentration, is not.Complexes, as the term is used here, also include compounds such assodium perborate, in which the elements of peroxide are reported to bean integral part of the molecule. The complexes according to thisinvention do not include persulfates or monopersulfates, such aspotassium monopersulfate (KHSO₅), which are found to be ineffective. Itis believed that the stability oxygen-sulfur bond in the persulfate isso great that persulfates cannot provide the elements of hydrogenperoxide needed for this synthesis. Apart from these stipulations,nothing is implied as to the structure of the complexes. They may becombinations of hydrogen peroxide with the inorganic compound or organicmolecule in which the peroxide is associated through weak or strongbonds. Alternatively, they may be reaction products of peroxide with thecompound or molecule, in which elements of the peroxide are incorporatedin the structure of the compound or molecule, but are available forreaction with acid halides. For some complexes, the structures may beunknown. It is preferable that the complexes be dry. It is morepreferable that the complexes be anhydrous. The term “dry” meansessentially free of water, though waters of crystallization may bepresent. “Anhydrous” means essentially free of water including waters ofcrystallization. A number of peroxide complexes and their syntheses aredescribed in U.S. Pat. No. 5,820,841.

[0019] It is preferred for the peroxide complex to be substantiallyinsoluble in the compatible aprotic solvent and to be present during thereaction as a solid phase. Such peroxide complexes are easily removedafter reaction by filtration or used in the form of a bed through whichthe acyl halide in compatible aprotic solvent is passed. Similarly, itis also preferred that the spent complex after reaction remain insolubleand in the solid phase.

[0020] Among the convenient inorganic peroxide complexes for thesynthesis of diacyl peroxides according to this invention arepercarbonate and perborate salts. These are most readily available asthe sodium salts, which are used in the detergent industry. The otheralkali metal salts of percarbonate or perborate, as for example, thepotassium salts may also be used in accordance with this invention.Those skilled in the art will recognize that the alkaline earthpercarbonates and perborates, as for example, the calcium salts, thoughless desirable because less readily available, would be expected to beuseful according to the processes of this invention. For the purposes ofthis invention, although both the alkali metal and alkaline earthpercarbonates and perborates have utility in the synthesis of diacylperoxides, the alkali metal salts are preferable, and the sodium saltsare more preferable. For convenience, the percarbonate salts andperborate salts will be referred to herein simply as percarbonate andperborate.

[0021] Sodium percarbonate, Na₂CO₃•1½H₂O₂, is hydrolyzed by moisture,and for best results in the synthesis of diacyl peroxide according tothis invention, the percarbonate should be kept dry. Sodium perborate,though represented as NaBO₃•H₂O and sometimes called sodium perboratemonohydrate, is reported to be Na₂(B₂O₈H₄), and is therefore ananhydrous salt. Analogously, the so-called sodium perborate tetrahydrateis reported to be the trihydrate: Na₂(B₂O₈H₄)•3H₂O. The misnamed sodiumperborate monohydrate is the preferred form to be used in the practiceof this invention.

[0022] The organic peroxide complexes useful for carrying out thisinvention include those that may have some solubility in the compatibleaprotic solvents, or at least be volatile enough to make separation fromthe compatible aprotic solvents difficult. The preferred organiccomplexes are those that are insoluble and whose residues are insolublein the compatible aprotic solvents, and which are present during thesynthesis as a solid phase. As such, they are easily separated from thediacyl peroxide solution. It is further desirable that the organiccomplexes be free of labile atoms or groups, or of bonds that can reactwith the reactants or products of the processes according to thisinvention, especially if such reactions degrade the organic molecule andsuch degradation products get into the reaction mixture.

[0023] Urea/hydrogen peroxide adduct (urea•H₂O₂) is a preferred organicperoxide complex. It is commercially available (Aldrich Chemical Co.,Milwaukee Wis., USA). It is a solid and is essentially insoluble in thesolvents designated herein and should small amounts be carried throughfilters or by other means into the diacyl peroxides solution, urea, notbeing active toward free-radical chain transfer, will have little effecton polymerization.

[0024] A significant advantage of the organic peroxide complexes is thatthey introduce no metal ions into reaction mixture and therefore givediacyl peroxide free of metal ions. In polymerization, such diacylperoxide will introduce no metal ions into the polymer. Polymers,especially fluoropolymers, of low metal content, or free of metal ions,are needed for certain applications where high purity is required, suchas the semiconductor industry.

[0025] An important characteristic of percarbonate, perborate, andurea/hydrogen peroxide adduct, and of the carbonate, borate, and urearemaining after their reaction, is their low solubility in thecompatible aprotic solvents that are used in this invention and becausethey are in the solid phase under the reaction conditions. Because theyare solids, they can be easily separated from reaction mixtures byfiltration. For the same reason, percarbonate, perborate, andurea/hydrogen peroxide adduct may be used in beds for continuoussynthesis of diacyl peroxides.

[0026] It is one of the advantages of the diacyl peroxide synthesis inaccordance with this invention that any aprotic solvent or mixturethereof may be used that dissolves the organic acyl halide and theproduct diacyl peroxide, and is not otherwise incompatible with theproduct diacyl peroxide, or the reactants, the organic acyl halide andthe percarbonate, or perborate, or urea/hydrogen peroxide adduct.Incompatible solvents include tertiary amines, because these can reactwith acyl halides and diacyl peroxides to form ammonium salts. Usefulsolvents include nonhalogenated solvents, and halocarbon solvents. Inthe class of nonhalogenated solvents are hydrocarbon solvents. Thesehave utility in diacyl peroxide solutions that are used inpolymerization of hydrocarbon monomers, but they are less useful for thepolymerization of fluoromonomers because of the chain transfer activitycharacteristic of hydrocarbons in fluoromonomer polymerization.Halocarbon solvents, because of their low chain transfer activity, aretherefore preferred because of their utility in both fluoromonomer andhydrocarbon monomer polymerizations.

[0027] Among the non-halogenated solvents, carbon dioxide in its liquidor supercritical states is preferred. It does not undergo chaintransfer, is not reactive toward oxidizing agents such as diacylperoxide, and being a gas at atmospheric pressure and room temperature,is easily removable from the products of polymerization. Surprisingly,it has been found that carbon dioxide, a Lewis acid, is an effectivesolvent for the production of diacyl peroxide by the reaction of acylhalides with peroxide complexes. This discovery provides a route to thedirect synthesis in good yield of diacyl peroxides in carbon dioxide,minimizing the presence of water and eliminating any organic solventsuch as would be inevitable in synthetic routes that would prepare thediacyl peroxide first in another solvent, subsequently replacing thatsolvent, by whatever means, with carbon dioxide. Carbon dioxidesolutions of diacyl peroxide find particular utility in polymerizationsconducted in carbon dioxide, because such initiator solution does notintroduce a second solvent into the polymerization.

[0028] The halocarbon solvents include fluorocarbons,hydrofluorocarbons, hydrochlorofluorocarbons, chlorofluorocarbons,perhalocarbons, and perfluorocarbons. It is preferred that the in thehydrogen-containing halocarbon solvents, the hydrogens be non-labile,that is that they not be susceptible to significant chain-transfer inthe presence of free radicals, especially during polymerization offluoroolefins. Also useful are “halocarbon ethers”, which are definedhere as molecules containing at least one ether linkage in which thecarbon atoms adjacent to the ether oxygen are completely halogenated,preferably completely fluorinated, or substituted with alkyl groups,preferably halogenated alkyl groups, and the monovalent atoms on theremaining carbon atoms being independently hydrogen, fluorine, orchlorine. Another class of useful solvents is perfluoroamines. Incontrast to organic amines that are not fluorinated, the perfluoroamineshave little or no basic character. Preferred compatible aprotic solventsare halocarbons, more preferably chlorofluorocarbons such as liquidCF₂Cl-CFCl₂ (CFC-113) and fluorocarbons such as liquidCF₃CF₂CF₂OCF(CF₃)CF₂OCFHCF₃ available as Fluoroether E2 from LancasterSynthesis Inc., Windham, N.H., USA.

[0029] One of the unique aspects of this invention is that it permitsdirect production of diacyl peroxide in the solvent or solvents ofchoice without any trace of other solvent.

[0030] Because peroxide initiators are generally made, stored, and usedin solution, it is desirable to choose a solvent that will not interferewith the polymerization reaction, as for example by undesiredchain-transfer reactivity. It is better still if the initiator solventis the same as the polymerization solvent. Then, with only a singlesolvent in the polymerization system, solvent removal and purificationat the end of the reaction (for batch polymerizations) or in the recycleloop (for continuous polymerizations) is simplified.

[0031] The process according to this invention is substantially free ofcompounds that are oxidizable by the peroxide complex or by products ofthe reaction of organic acyl halide with peroxide complex, i.e.,intermediate products or diacyl peroxide, under the conditions of thereaction. The identity of such compounds is known to those skilled inthe art. Such materials include olefinic and acetylenic compounds,thiols, sulfides, disulfides, and other oxidizable sulfur compounds,alcohols, aldehydes, and ketones, and amines and other oxidizablenitrogen compounds. At low concentration, oxidizable compounds willdecrease the yield of diacyl peroxide and may introduce undesirableimpurities into the product that will affect subsequent polymerization.At higher concentrations, the presence of oxidizable compounds may makethe reaction difficult to control and lead to excessive heat generation.By “substantially free” is meant that the oxidizable compounds arepresent in amounts that reduce the diacyl peroxide yield obtainable inthe absence of the oxidizable compounds by no more than 50%, preferablyby no more than 25%, more preferably by no more than 10%, and still morepreferably by no more than 5%, and most preferably by no more than 1%.

[0032] As stated above, it is an advantage of this invention that diacylperoxide is made without using aqueous alkaline peroxide solution, incontrast to the classical synthetic method. An aqueous phase ispreferably not part of the process of this invention. Preferably, waterper se is not added to the reaction. The presence of water will notcompletely prevent the production of diacyl peroxide but water willpromote the formation of organic acid, (by hydrolysis of the organicacyl halide), and of peracid and/or organic acid (by hydrolysis of thediacyl peroxide). In addition, water that remains in the diacyl peroxidecan cause corrosion in the polymerization equipment, particularlythrough hydrolysis of acid halides to produce hydrogen chloride andhydrogen fluoride. Water will also complicate the removal andpurification of the polymerization solvent. These disadvantages causedby the presence of water become greater if enough water is present for aseparate aqueous phase to form. Preferably, the amount of water islimited so as to prevent formation of a separate aqueous phase. Forthese reasons, care should be taken in the synthesis of diacyl peroxidesaccording to this invention to have dry equipment and to keep theingredients dry. If the reagents or the equipment is not completely dry,adding desiccants such as Drierite® (anhydrous calcium sulfate) to thereaction mixture may increase diacyl peroxide yield.

[0033] The temperature of the reaction is chosen to balance the interestin having a fast reaction, with the need to prevent loss of diacylperoxide through thermal decomposition. Because diacyl peroxides vary inhalf-life (the time for one-half of the peroxide to be consumed; afunction of temperature), reaction temperatures will vary, but usefultemperatures are in the range of about −40° C. to about 40° C. Fordiacyl peroxides such as HFPO dimer peroxide, heptafluorobutyrylperoxide, isobutyryl peroxide, and bis[perfluoro(fluorosulfonyl)acetyl]peroxide, a temperature range of about −20° C. to about 20° C. istypical, about −10° C. to about 10° C. is preferred, and about −5° C. toabout 5° C. is more preferred when sodium percarbonate or sodiumperborate is used. When urea/hydrogen peroxide adduct is used to makethese diacyl peroxides, about 0° C. to about 10° C. is the morepreferred temperature. Diacyl peroxide loss to thermal decomposition isbest minimized by keeping reaction time a fraction of the diacylperoxide's half-life at reaction temperature. A reaction time no greaterthan one-quarter of the diacyl peroxide half-life at the reactiontemperature is preferred.

[0034] Because residual acyl halide is an impurity in the product diacylperoxide, and is furthermore a source of acid that can cause corrosion,it is desirable to conduct the synthesis so as to yield as much of thediacyl peroxide as possible. Yield is preferably at least about 25%,more preferably at least about 50%, more preferably still at least about70%, and most preferably at least about 90%.

[0035] When diacyl peroxide is synthesized according to this inventionin a batchwise manner, the reactant organic acyl halide is mixed incompatible aprotic solvent with peroxide complex. Surprisingly, it isfound that the yield of diacyl peroxide increases as the mole ratio ofperoxide in the peroxide complex to acyl halide increases. It ispreferable that the mole ratio be at least about one to one. It is morepreferable that the mole ratio be at least about two to one. It is mostpreferable that the mole ratio be at least about four to one. Becausethe peroxide content of the peroxide complex depends upon the nature ofthe complex, the weight of complex that contains a mole of peroxide orits equivalent will depend upon the composition of the complex beingconsidered.

[0036] To prepare diacyl peroxide in a continuous reaction according tothis invention, a feed stream comprised of organic acyl halide incompatible aprotic solvent is continuously contacted with a bedcomprised of peroxide complex, in the absence of organic compoundssusceptible to oxidation under the reaction conditions to form a productstream comprising diacyl peroxide in compatible aprotic solvent. The bedmay be in the form of a column filled with peroxide complex andoptionally an inert material. The purpose of the inert material would beto facilitate flow and temperature control. As stated above, thesynthesis should be run so as to achieve high yield of the diacylperoxide. The continuous method is preferred because it allows diacylperoxide to be made as needed and consumed promptly. If desired, thediacyl peroxide in compatible aprotic solvent can be collected andadvantageously used directly in that form. The continuous processensures that fresh diacyl peroxide is always available and eliminatesthe need for diacyl peroxide storage, which generally requires lowtemperatures, and is therefore vulnerable to power outages and equipmentfailure. Furthermore, as with any oxidizing agent, it is sound practiceto minimize the quantities of diacyl peroxide kept on hand. Both batchand continuous methods are demonstrated in the Examples.

EXAMPLES GLOSSARY

[0037] HFPO=Hexafluoropropylene oxide

[0038] HFPO Dimer Peroxide=

CF₃CF₂CF₂OCF(CF₃)(C═O)OO(C═O)(CF₃)CFOCF₂CF₂CF₃

[0039] HFPO Dimer Acid Fluoride=CF₃CF₂CF₂OCF(CF₃)(C═O)F

[0040] DAF=HFPO Dimer Acid Fluoride

[0041] CFC-113=CF₂Cl-CFCl₂

[0042] Vertrel® XF=CF₃CFHCHFCF₂CF₃ (2,3-dihydroperfluoropentane)available from the DuPont Company, Wilmington, Del., USA

[0043] Fluoroether E2=CF₃CF₂CF₂OCF(CF₃)CF₂OCFHCF₃(2H-Perfluoro-5-methyl-3,6-dioxanonane) available from LancasterSynthesis Inc., Windham, N.H., USA

TEST METHOD

[0044] Diacyl peroxides formed by this process are analyzed by peroxidetitration using the following standard procedure. In a loosely stopperedErlenmeyer flask, several grams of dry ice are added to 25 ml of glacialacetic acid, thereby flushing oxygen from the system. 5.0 ml of asolution of 30 g of potassium iodide in 70 ml of deoxygenated water isadded, and then 5.0 ml of the peroxide solution to be analyzed is added.The mixture is stirred for 30 minutes to allow the peroxide to reactwith the iodide. 100 ml of deoxygenated water is added and the reactionmixture, having a deep iodine color, is titrated to light yellow with0.1 N sodium thiosulfate. Then 0.5 g of Thyodene® (Fisher ScientificCo.) iodometric indicator is added making the reaction mixture turnblue. Titration is continued with 0.1N sodium thiosulfate to a colorlessendpoint. The molar peroxide concentration is 0.01 times the totalnumber of ml of 0.1N sodium thiosulfate solution added to the reaction.

EXAMPLE 1 HFPO Dimer Peroxide Synthesis in CFC-113 Using SodiumPercarbonate

[0045] A round-bottom flask is charged with 50 ml CFC-113 and 2.0 g ofdry sodium percarbonate (13 mmoles of sodium percarbonate, or 19 mmolesof H₂O₂ equivalent). After chilling the contents of the flask to 0° C.,5.2 ml (25 mmole) of HPFO dimer acid fluoride (DAF) is added and theresulting slurry is stirred magnetically for 3 hours. The reactionmixture is filtered through a pad of Drierite® on glass wool, anoperation assumed to remove any unreacted sodium percarbonate and anyfree H₂O₂. The filtrate is titrated and found to be 0.18 M in peroxide.Assuming a product volume of 55 ml, this is 9.9 mmole of peroxide or a79% yield based on the starting organic acyl fluoride, DAF.

EXAMPLE 2 HFPO Dimer Peroxide Synthesis in CFC-113 Using SodiumPerborate

[0046] A slurry of 4.9 g sodium perborate monohydrate (49 mmoles,Aldrich) in 75 ml of CFC-113 is stirred magnetically in a round-bottomflask under a positive pressure of nitrogen. The flask is immersed in awet ice bath and, once its contents have chilled, 5.2 ml of HFPO dimeracid fluoride (25 mmoles) is added with stirring. The contents of theflask are stirred for 3 hours at 2° C. to 6° C. The reaction mixture isvacuum filtered, the filter pad rinsed with CFC-113, and the filtrateimmediately washed through 25 g Drierite® with additional CFC-113.Passage through the Drierite® makes the solution noticeably hazy. Thisgives 69 ml of HFPO dimer peroxide solution that titrated 0.12 M inperoxide (66% yield). The next morning the product is washed three timeswith 50 ml of water and retitrated, coming out 0.13 M in peroxide (someof the CFC-113 may have evaporated in the washing process, increasingperoxide concentration).

EXAMPLE 3 HFPO Dimer Peroxide Synthesis in CFC-113 Using Hydrated SodiumPerborate

[0047] A slurry of 7.7 g sodium perborate tetrahydrate (50 mmoles,Aldrich) in 75 ml of CFC-113 is stirred magnetically in a round-bottomflask under a positive pressure of nitrogen. The flask is immersed in awet ice bath and, once its contents are chilled, 5.2 ml of HFPO dimeracid fluoride (25 mmoles) is added with stirring. The contents of theflask are stirred for 3 hours at 2° C. to 5° C. The reaction mixture wasvacuum filtered, the filter pad rinsed with CFC-113, and the filtrateimmediately washed through 25 g Drierite® with additional CFC-113.Passage through the Drierite® made the solution noticeably hazy. Thisgave 74 ml of HFPO dimer peroxide solution that titrates as 0.042 M inperoxide (25% yield). The next morning the product is washed three timeswith water and retitrated, coming out 0.046 M in peroxide (some of theCFC-113 may have evaporated in the washing process, increasing peroxideconcentration).

[0048] The sodium perborate tetrahydrate, though effective in thissynthesis, shows reduced yield of the dimer peroxide. This indicatesthat the presence of water is deleterious for the reaction. It ispointed out in the detailed description of the invention that sodiumperoxide monohydrate is actually an anhydrous salt, and that sodiumperborate tetrahydrate is in fact a trihydrate. The addition of a dryingagent, such as Drierite®, might improve the yield by taking up the waterintroduced by the hydrated sodium perborate.

EXAMPLES 4-8 Influence of Ratio of Percarbonate to Acyl Halide

[0049] The experimental conditions of Example 1 are followed except thatin place of CFC-113, the reaction solvent is Fluoroether E2, andconcentrations of sodium percarbonate and DAF are varied to determinethe effect of the ratio on product yield. Temperatures are maintained at0° C. Results are summarized in Table 1. The 104% yield result may bedue to evaporation of solvent in the course of analysis, or it may beexperimental error. TABLE 1 Mole Ratio Example Percarbonate DAF ReactionTime Yield 4 1 1 3 hrs 61% 5 1.5 1 3 hrs 79% 6 2 1 3 hrs 89% 7 4 1 3 hrs104%  8 1.5 1 0.5 hrs   31%

[0050] Examples 4 to 8 show that increasing the ratio of percarbonate toacyl halide increases yield. This is contrary to the prior art (McKillopand Sanderson, p. 6152) as well as to expectations based on thestoichiometry of the reaction. Equation (2) shows the desired reactionbetween the peroxide complex, represented simply as hydrogen peroxide,and acyl halide:

H₂O₂+2R(C═O)X→R(C═O)—O—O(C═O)R+2HX   (2)

[0051] The competing, undesirable reaction is the formation of peracid,shown in Equation (3):

H₂O₂+R(C═O)X→R(C═O)—O—OH+HX   (3)

[0052] Increasing the ratio of peroxide to acyl halide should increasethe reaction of Equation (3), and decrease that of Equation (2).Surprisingly, the reverse is observed.

EXAMPLE 9 Isobutyryl Peroxide Synthesis

[0053] A round-bottom flask is charged with 50 ml of CFC-113 and 2.0 gof sodium percarbonate (13 mmoles or 19 mmoles of H₂O₂ equivalent).After chilling the contents of the flask to 0° C., 2.60 ml of isobutyrylchloride (25 mmoles) is added and the resulting slurry is stirredmagnetically for 223 minutes. The reaction mixture is filtered through apad of Drierite® on glass wool, washing through with fresh CFC-113. Thefiltrate, now measuring 59 ml in volume, is found to be 0.083 M inperoxide, which is a 39% yield based on starting isobutyryl chloride.The peroxide solution is washed three times with ˜60 ml of water. Thewashed solution is retitrated and found to be 0.050 M in peroxide. Thewater wash may have removed residual inorganic peroxide missed by theDrierite® filtration, but is more likely that some of the isobutyrylperoxide was destroyed by hydrolysis.

[0054] This example shows that the process of this invention can be usedto prepare hydrocarbon acyl peroxides as well as fluorocarbon acylperoxides.

EXAMPLE 10 Heptafluorobutyryl Peroxide Synthesis

[0055] A round-bottom flask is charged with 50 ml of CFC-113 and 2.0 gof sodium percarbonate (13 mmoles or 19 mmoles of H₂O₂ equivalent).After chilling the contents of the flask to 0° C., 3.73 ml ofheptafluorobutyryl chloride (25 mmoles) is added and the resultingslurry is stirred magnetically for 3.3 hours. The reaction mixture isfiltered through a pad of Drierite® on glass wool, washing through withfresh CFC-113, an operation assumed to remove any unreacted percarbonateand any free H₂O₂. The filtrate, now measuring 45 ml in volume, is foundto be 0.10 M in peroxide for a 37% yield based on startingheptafluorobutyryl chloride. In order to make sure that all of thesodium percarbonate and hydrogen peroxide has been removed by filtrationthrough Drierite®, the peroxide solution is washed three times with45-50 ml of water. On retitration, the solution is found to still be0.10 M in peroxide.

EXAMPLE 11 Bis[perfluoro(fluorosulfonvylacety] Peroxide Synthesis

[0056] A round-bottom flask is charged with 50 ml of CFC-113 and 2.0 gof sodium percarbonate (13 mmoles or 19 mmoles of H₂O₂ equivalent).After chilling the contents of the flask to 0° C., 2.83 ml ofFSO₂CF₂(C═O)F (25 mmoles) is added and the resulting slurry is stirredmagnetically for 3 hours. The reaction mixture is filtered through a padof Drierite® on glass wool, washing through with fresh CFC-113, anoperation assumed to remove any unreacted percarbonate and any freeH₂O₂. The filtrate, now measuring 52 ml in volume, is found to be 0.10 Min peroxide for a 42% yield based on starting FSO₂CF₂(C═O)F.

[0057] This example shows that acyl halides with hydrolyzable functionalgroups can be converted by the method of this invention to diacylperoxides, without affecting the hydrolyzable functional group.

EXAMPLE 12 HFPO Dimer Peroxide Synthesis in CFC-113 Using Urea HydrogenPeroxide Adduct

[0058] A round bottomed flask under a positive pressure of nitrogen gasis charged with 75 ml of CFC-113, 2.65 g of Na₂CO₃ (25 mmole), 2.35 gurea/hydrogen peroxide adduct (25 mmoles, H₂NCONH₂•H₂O₂), and 5.2 ml ofHFPO dimer acid fluoride (25 mmole) with ice bath cooling. The reactionmixture is stirred for 3 hours at −7° C. to 2° C. (mostly at 1° C. to 2°C.), washed though a vacuum filter with CFC-113, and washed through 25 gof Drierite® in a chromatography column with CFC-113. This gives 97 mlof CFC-113 solution that titrates 0.046 M in peroxide (37% yield). Afterwashing the CFC-113 solution three times with ice water, it stilltitrates 0.046M in peroxide.

EXAMPLE 13 HFPO Dimer Peroxide Synthesis In Liquid Carbon Dioxide

[0059] A 300 ml stainless steel autoclave, equipped with a paddlestirrer and dip tube, is dried by heating to 100° C. for several hoursunder a dry nitrogen purge. Dry sodium percarbonate (Na₂CO₃•1½H₂O₂)(2 g(12.7 mmol)) is added and the autoclave is sealed, evacuated, and cooledto about −20° C.

[0060] Separately, a 1-liter stainless steel cylinder is charged with5.2 ml (24.7 mmol) of HFPO dimer acid fluoride (DAF). The cylinder iscooled on dry ice and evacuated, and about 220 g of carbon dioxide isadmitted. The cylinder is then connected to the autoclave using ⅛ inch(3.2 mm) diameter stainless steel tubing. The cylinder is inverted totransfer the entire contents of the cylinder to the autoclave. Priorvacuum of the autoclave and prior chilling of the autoclave promotesgood transfer. About 199 g of the HFPO dimer acid fluoride/liquid carbondioxide mix is transferred from the stainless steel cylinder into theautoclave.

[0061] The contents of the autoclave are stirred at about 5000 rpm forfour hours at 0° C. Temperature fluctuates mildly during this time from−2° C. to 0.5° C. The internal pressure in the autoclave varies from 477psi (3.29 MPa) at −2° C. to 520 psi (3.59 MPa) at 0.5° C. After aboutfour hours, the autoclave is chilled to −27° C. with the contents stillstirring. Chilling to −27° C. reduces the internal pressure of theautoclave to 184 psi (1.27 MPa). A 1-liter pressure-resistant cylinderis evacuated and cooled in a liquid nitrogen bath. The cylinder is thenconnected to the dip tube outlet on the autoclave using an 18 inch (45cm) length of ⅛ inch (3.2 mm) diameter stainless steel tubing. Thecontents of the autoclave are then vented into the stainless steelcylinder through the dip tube. At the end of the transfer, the pressurein the cylinder is 0.2 atm (20 kPa). A valve on the top of the cylinderis removed and 100 ml of Vertrel® XF is added so that the diacylperoxide in the carbon dioxide can be transferred in the Vertrel® XF tofacilitate measurement of reaction yield. The valve is replaced on thecylinder. The cylinder is removed from the liquid nitrogen bath.Contents of the cylinder are allowed to warm until rapid carbon dioxideevolution ceases. Evolution of carbon dioxide is judged by periodicallyopening and closing the cylinder valve and noting pressure changes.

[0062] Once carbon dioxide is no longer being rapidly evolved and froston the sides of the cylinder shows the first signs of thawing (about30-45 minutes), the valve is removed from the top of the cylinder.Contents of the cylinder, a hazy gray/blue fluid, are poured into apolyethylene bottle chilled on dry ice.

[0063] Opening the 300 ml autoclave at this point reveals residual whitesolid on the bottom and traces of white film on the walls of theautoclave. On visual inspection, the amount of solids left in theautoclave is observed to be approximately the same volume as the amountof sodium percarbonate added at the start.

[0064] The gray/blue fluid recovered from the reactor measures 85 ml involume. Peroxide titration of 5.0 ml takes 5.95 ml of 0.1 N thiosulfate.This titration corresponds to a 41% yield of HFPO dimer peroxide.

[0065] The remaining gray/blue fluid, measuring 80 ml, is warmed from−78° C. to room temperature and washed three times in a separatoryfunnel with water. This water wash removes any unreacted sodiumpercarbonate and hydrogen peroxide that would titrate the same as theHFPO dimer peroxide. A 5 ml aliquot of the solution now takes 6.40 ml of0.1 N thiosulfate in peroxide titration (the increase in peroxideconcentration may reflect some evaporation of the Vertrel® XF solventduring the water wash).

EXAMPLE 14 Continuous Synthesis of HFPO Dimer Peroxide in Liquid CarbonDioxide

[0066] A 150 ml stainless steel cylinder is evacuated and charged with7.90 g of perfluoro(2-methyl-3-oxa-hexanoyl) fluoride(CF₃CF₂CF₂OCF(CF₃)COF) (“DAF”) and 50 g carbon dioxide. The cylinder,equipped with a pressure gauge is inverted and placed in a stand fixedto a balance. {fraction (1/16)} inch (1.6 mm) diameter stainless steeltubing is connected from the cylinder to the top of a stainless steelcolumn about 0.56 cm in diameter and 10 cm in length. The column ispacked with 10.0 g of sodium percarbonate. A plug of glass wool at thebottom of the column keeps the sodium percarbonate in the column. Thecolumn is immersed in a constant temperature bath at 0° C. A shortlength of {fraction (1/16)} inch (1.6 mm) stainless steel tubing runsfrom a valve at bottom of the column, through a rubber septum, and intoa cold trap that is immersed in a dry-ice/acetone slurry and vented tothe atmosphere. The trap contains about 50 g Vertrel® XF.

[0067] The cylinder valve is opened allowing the liquid DAF/CO₂ mixtureto fill the column. The valve between the bottom of the column and thecold trap is then opened slightly to permit a controlled flow ofmaterial through the column at a rate of 0.154 g/min. The void volume inthe column is 6.0 ml. The void volume divided by the flow rate ofmaterial through the column is taken as the contact time. The contacttime is 39 minutes. The non-volatile effluent from the column is takenup in the cold trap to form a solution in Vertrel®XF. The lowtemperature of the trap preserves the diacyl peroxide formed, and thesolvent provides a convenient medium for subsequent product analysis.Most of the CO₂ is vented spontaneously to the atmosphere from the trap.At the conclusion of the experiment, the cold trap is warmed to 0° C. inice water and vigorously agitated until the weight of the trap remainsconstant to remove any remaining CO₂. Peroxide titration of aliquots ofsolution from the cold trap shows that 4.81 g of peroxide is formed. Itsidentity is confirmed from absorption at 1858 cm⁻¹ and 1829 cm⁻¹ in itsinfrared spectrum arising from carbonyl groups in the diacyl peroxide.The amount of DAF remaining in the collected product is 2.19 g asdetermined from the intensity of the infrared absorption at 1881 cm⁻¹arising from the acid fluoride carbonyl group. From these data yield ofperoxide is calculated to be 68.7%.

EXAMPLE 15 Continuous Synthesis of HFPO Dimer Peroxide in Liquid CarbonDioxide

[0068] The procedure and equipment are as described in Example 14 exceptthe 4.74 g DAF is charged in the cylinder, the feed rate is 0.129 g/min,and the contact time is 46 minutes. Product collected is 4.02 g, and0.67 g remains on the column. The product consists of 2.94 g peroxideand 1.41 g of recovered DAF. Yield is 67.6 %.

EXAMPLE 16 Continuous Synthesis of HFPO Dimer Peroxide in Liquid CarbonDioxide

[0069] The procedure and equipment are as described in Example 14. Thefeed rate is 0.0697 g/min, and the contact time is 86 minutes. Productcollected is 7.01 g and 1.53 g remain on the column. The productconsists of 6.23 g peroxide and 0.43 g of recovered DAF. Yield is93.56%.

EXAMPLE 17 Continuous Synthesis of HFPO Dimer Peroxide in Liquid CarbonDioxide

[0070] The procedure and equipment are as described in Example 14 exceptthe temperature of the bath around the column is maintained at 10° C.,the feed rate is 0.165 g/min, and the contact time is 32 minutes.Product collected is 5.87 g, and 1.89 g remains on the column. Theproduct consists of 5.36 g peroxide and 0.43 g of recovered DAF. Yieldis 91.3%.

EXAMPLE 18 Continuous Synthesis of HFPO Dimer Peroxide in Liquid CarbonDioxide

[0071] The procedure and equipment are as described in Example 14 exceptthe temperature of the bath around the column is maintained at 15° C.,the feed rate is 0.242 g/min, and the contact time is 20 minutes.Product collected is 5.92 g, and 1.69 g remains on the column. Theproduct consists of 5.13 g peroxide and 1.02 g of recovered DAF. Yieldis 83.4%.

Summary of Examples 14 to 18

[0072] Table 2 summarizes the results of the examples of the continuoussynthesis of diacyl peroxide. Yields are increased with longer contacttime or with higher reaction temperature. TABLE 2 Contact TimeTemperature Example (min) (° C.) Yield (%) 14 39 0 68.7 15 46 0 67.6 1686 0 93.6 17 32 10 91.3 18 20 15 83.4

EXAMPLE 19 HFPO Dimer Peroxide Synthesis In Carbon Dioxide Using UreaHydrogen Peroxide Adduct

[0073] A jacketed autoclave of 125 ml volume is heated to 60° C. andpurged with nitrogen for several hours. The autoclave is then cooled toroom temperature and 3.0 g (30.9 mmoles H₂O₂ equivalent) urea/hydrogenperoxide adduct (Aldrich Chemical Co.), containing 35.0% H₂O₂ byperoxide titration, is added under a stream of nitrogen. The autoclaveis closed, evacuated, and cooled to −20° C. A cylinder, into which 16.0g of HFPO dimer acid fluoride (48.2 mmoles) and 60 g of carbon dioxidehad been charged, is connected to the autoclave and the contents of thecylinder are transferred into the autoclave. The temperature of theautoclave is then raised to 0° C. while its contents are agitated for 6hrs. The bottom port of the autoclave is fitted with a sintered metalfilter containing 15 micrometer pores to retain urea and unusedurea/hydrogen peroxide adduct. The contents of the autoclave are ventedinto an accurately weighed nitrogen flushed cold trap immersed in a dryice/acetone bath. The trap contained about 50 g of Vertrel® XF. Thesolvent is used to absorb the reaction mixture as most of the carbondioxide is vented to the atmosphere. This also provided a convenientmedium for infrared analysis of the reaction mixture at room temperatureand atmospheric pressure.

[0074] The cold trap and its contents are warmed to 0° C. in an ice bathwith shaking to expel remaining carbon dioxide from the Vertrel® XFsolution. The trap is dried and weighed and used to determine the weightof the product solution obtained. A portion of the solution is thenplaced in a liquid infrared cell and its spectrum measured. A referencespectrum of Vertrel® XF previously obtained in the same liquid cell issubtracted from that of the product mixture and intensities of bandsoccurring at 1858 cm⁻¹ and 1829 cm⁻¹ for the HFPO dimer peroxide, 1880cm⁻¹ for the HFPO dimer acid fluoride and 1774 cm⁻¹ for the HFPO dimeracid are determined. Calibration curves determined from solutions ofknown concentration are used to calculate the amounts of each compoundfrom the intensity of the appropriate infrared band in the spectrum ofthe product mixture. We found 60.6% HFPO dimer peroxide, 36.5% HFPOdimer acid fluoride and 3.0% HFPO dimer acid in the product mixtureweighing 13.35 g.

EXAMPLE 20 HFPO Dimer Peroxide Synthesis In Carbon Dioxide Using UreaHydrogen Peroxide Adduct

[0075] The procedure given in Example 19 is used except the temperatureof the autoclave is raised to 5° C. We found 83.0% HFPO dimer peroxide,12.5% HFPO dimer acid fluoride and 4.5% HFPO dimer acid in the productmixture weighing 15.32 g.

EXAMPLE 21 HFPO Dimer Peroxide Synthesis In Carbon Dioxide Using UreaHydrogen Peroxide Adduct

[0076] The procedure given in Example 19 is used except the temperatureof the autoclave is raised to 10° C. and agitation is continued for 3hrs. We found 76.1% HFPO dimer peroxide, 15.5% HFPO dimer acid fluorideand 8.4% HFPO dimer acid in the product mixture weighing 12.36 g.

EXAMPLE 22 HFPO Dimer Peroxide Synthesis In Carbon Dioxide Using UreaHydrogen Peroxide Adduct

[0077] The procedure given in Example 19 is used except 2.9 g of urea isadded to the autoclave along with the urea/hydrogen peroxide adduct toserve as a mild base to absorb HF generated during the reaction. Thetemperature of the autoclave is also raised to 5° C. We found 81.4% HFPOdimer peroxide, 15.4% HFPO dimer acid fluoride and 3.2% HFPO dimer acidin the product mixture weighing 7.11 g.

EXAMPLE 23 HFPO Dimer Peroxide Synthesis In Carbon Dioxide Using UreaHydrogen Peroxide Adduct

[0078] The procedure given in Example 19 is used except the amount ofurea/hydrogen peroxide adduct charged to the autoclave is 5.0 g (51.5mmoles H₂O₂ equivalent) and the temperature of the autoclave is raisedto 5° C. We found 87.8% HFPO dimer peroxide, 6.4% HFPO dimer acidfluoride and 5.8% HFPO dimer acid in the product mixture weighing 16.39g.

Summary of Examples 19 to 23

[0079] Table 3 summarizes the results of the examples of the synthesisof diacyl peroxide using urea/hydrogen peroxide adduct. Yields areincreased with longer contact time or with higher reaction temperature.Increasing the ratio of urea/hydrogen peroxide adduct to acyl fluoride(DAF) increases yield. Added urea has little or no effect. TABLE 3Contact Time Temperature DAF:H₂O₂ Example (hour) (° C.) (mmoles) Yield(%) 20 6 0 48.2:30.9 47.2 21 6 5 48.2:30.9 83.0 22 3 10 48.2:30.9 76.1 23* 6 5 48.2:30.9 81.4 24 6 5 48.2:51.5 87.8

What is claimed is:
 1. A process for the synthesis of diacyl peroxidecomprising contacting organic acyl halide and peroxide complex incompatible aprotic solvent substantially free of compounds oxidizable bythe peroxide complex or by products of the reaction of organic acidhalide with peroxide complex.
 2. The process of claim 1 furthercomprising collecting compatible aprotic solvent containing diacylperoxide.
 3. The process of claim 1 further comprising limiting theamount of water present so as to prevent formation of an aqueous phase.4. The process of claim 1 wherein the peroxide complex is substantiallyinsoluble in said compatible aprotic solvent and is present as a solidphase.
 5. The process of claim 1 wherein the peroxide complex isselected from the group consisting of sodium percarbonate, sodiumperborate, and urea/hydrogen peroxide adduct and mixtures thereof. 6.The process of claim 1 wherein the mole ratio of peroxide in theperoxide complex to organic acyl halide is at least about one-to-one. 7.The process of claim 1 wherein the process is carried out at a reactiontemperature between about −40° C. and about 40° C.
 8. The process ofclaim 1 wherein the process is carried out at a reaction temperaturebetween about −20° C. and about 20° C.
 9. The process of claim 1 whereinthe process is carried out at a reaction temperature between about −10°C. and about 10° C.
 10. The process of claim 1 wherein the process iscarried out at a reaction temperature selected so that the reaction timeis no greater than one-quarter of the diacyl peroxide half-life at thereaction temperature.
 11. The process of claim 1 wherein the organicacyl halide is selected from the group consisting of fluoroorganic acylhalides.
 12. The process of claim 1 wherein the organic acyl halide isselected from the group consisting of perfluoroorganic acyl halides. 13.The process of claim 1 wherein the organic acyl halide is isobutyrylhalide.
 14. The process of claim 1 wherein the compatible aproticsolvent is selected from the group consisting of a halocarbon,chlorofluorocarbon hydrochlorofluorocarbon, hydrochlorocarbon,hydrofluorocarbon, perfluorocarbon, halocarbon ether and mixturesthereof.
 15. The process of claim 1 wherein the compatible aproticsolvent is a nonhalogenated solvent.
 16. The process of claim 1 whereinthe compatible aprotic solvent is liquid or supercritical carbondioxide.
 17. A process for the continuous synthesis of diacyl peroxidescomprising continuously contacting a feed stream comprised of organicacyl halide in compatible aprotic solvent with a bed comprised ofperoxide complex to form a product stream comprised of diacyl peroxidein compatible aprotic solvent, said compatible aprotic solvent beingsubstantially free of compounds oxidizable by peroxide complex or byproducts of the reaction of organic acid halide with peroxide complex.18. The process of claim 17 further comprising collecting said productstream.
 19. The process of claim 17 further comprising limiting theamount of water present so as to prevent formation of an aqueous phase.